For the following reaction, 6.10 grams of silver nitrate are mixed with excess copper(II) chloride. The reaction yields 4.77 grams of silver chloride
What is the theoretical yield of silver chloride? What is the percent yield of silver chloride?
CuCl2 + 2AgNO3 --> Cu(NO3)2 + 2AgCl
to three places:
moles AgNO3 = grams/molar mass = 6.10/170 = 0.0359
moles AgCl formed = 2*0.0359/2 = 0.0359
g AgCl formed = moles AgCl x molar mass AgCl = 0.0359*143 = 5.13 g = theoretical yield = TY
Actual yield from problem = AY = 4.77 g.
% yield = (AY/TY)*100 = ?
To determine the theoretical yield of silver chloride, we need to calculate the amount of silver chloride that would be produced if the reaction went to completion.
First, we need to balance the chemical equation for the reaction:
AgNO3 + CuCl2 -> AgCl + Cu(NO3)2
From the balanced equation, we can see that the stoichiometric ratio of AgNO3 to AgCl is 1:1. This means that for every 1 mole of AgNO3, we would expect to form 1 mole of AgCl.
Next, we need to convert the mass of AgNO3 to moles. To do this, we divide the given mass of AgNO3 (6.10 grams) by its molar mass. The molar mass of AgNO3 can be calculated by adding up the atomic masses of each element in the compound, which are:
Ag (silver) = 107.87 g/mol
N (nitrogen) = 14.01 g/mol
O (oxygen) = 16.00 g/mol (x3 as there are three oxygen atoms in AgNO3)
Molar mass of AgNO3 = 107.87 + 14.01 + (16.00 x 3) = 169.87 g/mol
Now we can calculate the number of moles of AgNO3:
moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3 = 6.10 g / 169.87 g/mol
Next, since the stoichiometric ratio of AgNO3 to AgCl is 1:1, we know that the number of moles of AgCl formed will be the same as the number of moles of AgNO3:
moles of AgCl = moles of AgNO3
Finally, to calculate the theoretical yield of AgCl, we multiply the number of moles of AgCl by its molar mass. The molar mass of AgCl can be calculated using the atomic masses of Ag and Cl:
Ag (silver) = 107.87 g/mol
Cl (chlorine) = 35.45 g/mol
Molar mass of AgCl = 107.87 + 35.45 = 143.32 g/mol
theoretical yield of AgCl = moles of AgCl x molar mass of AgCl
To determine the percent yield of AgCl, we need to compare the actual yield (4.77 grams) to the theoretical yield we just calculated and calculate the percentage:
percent yield = (actual yield / theoretical yield) x 100
Now you can plug in the values and calculate the theoretical yield and percent yield of AgCl.
To calculate the theoretical yield of silver chloride, we need to determine the stoichiometry of the reaction between silver nitrate and copper(II) chloride.
From the balanced chemical equation:
2 AgNO3 + CuCl2 -> 2 AgCl + Cu(NO3)2
We can see that for every 2 moles of AgNO3, we produce 2 moles of AgCl.
First, let's convert the given mass of AgNO3 to moles:
Molar mass of AgNO3 = 107.87 g/mol + 14.01 g/mol + (3 * 16.00 g/mol) = 169.87 g/mol
Moles of AgNO3 = mass / molar mass = 6.10 g / 169.87 g/mol = 0.036 moles
Since the stoichiometry is 2:2, the same number of moles of AgCl will be produced.
The molar mass of AgCl is 107.87 g/mol + 35.45 g/mol = 143.32 g/mol
The theoretical yield of AgCl = moles of AgCl * molar mass of AgCl = 0.036 moles * 143.32 g/mol = 5.16 grams
To calculate the percent yield, we need the actual yield, which is given as 4.77 grams.
Percent yield = (actual yield / theoretical yield) * 100
= (4.77 g / 5.16 g) * 100
= 92.44%
Therefore, the theoretical yield of silver chloride is 5.16 grams, and the percent yield is 92.44%.